Na2CrO4 → 2Na+ + CrO42−
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- Electrolytic dissociation of sodium chromate
Electrolytic dissociation of sodium chromate yields sodium ion and chromate ion. This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Electrolytic dissociation of sodium chromate
General equation
- Electrolytic dissociation of salt
- SaltLewis conjugate ⟶ CationLewis acid + AnionLewis base
Oxidation state of each atom
- Electrolytic dissociation of sodium chromate
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Na2CrO4 | Sodium chromate | 1 | Lewis conjugate | Salt |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Na+ | Sodium ion | 2 | Lewis acid | Cation |
| CrO42− | Chromate ion | 1 | Lewis base | Anion |
Thermodynamic changes
Changes in standard condition
- Electrolytic dissociation of sodium chromate◆
ΔrG −16.63 kJ/mol K 8.19 × 102 pK −2.91
| Standard enthalpy of reaction ΔrH° kJ · mol−1 | Standard Gibbs energy of reaction ΔrG° kJ · mol−1 | Standard entropy of reaction ΔrS° J · K−1 · mol−1 | Standard heat capacity of reaction at constant pressure ΔrCp° J · K−1 · mol−1 | |
|---|---|---|---|---|
per 1 mol of Equation | −19.2 | −16.63 | −8.4 | – |
per 1 mol of | −19.2 | −16.63 | −8.4 | – |
per 1 mol of Sodium ion | −9.60 | −8.315 | −4.2 | – |
per 1 mol of Chromate ion | −19.2 | −16.63 | −8.4 | – |
Thermodynamic data of reactants
| Chemical formula | Standard enthalpy of formation ΔfH° kJ · mol−1 | Standard Gibbs energy of formation ΔfG° kJ · mol−1 | Standard molar entropy S° J · K−1 · mol−1 | Standard molar heat capacity at constant pressure Cp° J · K−1 · mol−1 |
|---|---|---|---|---|
| Na2CrO4 (cr) | -1342.2[1] | -1234.93[1] | 176.61[1] | 142.13[1] |
| Na2CrO4 (ai) | -1361.39[1] | -1251.58[1] | 168.2[1] | – |
| Na2CrO4 (cr) 4 hydrate | -2528.8[1] | – | – | – |
| Na2CrO4 (cr) 10 hydrate | -4281.1[1] | – | – | – |
* (cr):Crystalline solid, (ai):Ionized aqueous solution
Thermodynamic data of products
| Chemical formula | Standard enthalpy of formation ΔfH° kJ · mol−1 | Standard Gibbs energy of formation ΔfG° kJ · mol−1 | Standard molar entropy S° J · K−1 · mol−1 | Standard molar heat capacity at constant pressure Cp° J · K−1 · mol−1 |
|---|---|---|---|---|
| Na+ (g) | 609.358[1] | – | – | – |
| Na+ (ao) | -240.12[1] | -261.905[1] | 59.0[1] | 46.4[1] |
| CrO42− (ao) | -881.15[1] | -727.75[1] | 50.21[1] | – |
* (g):Gas, (ao):Un-ionized aqueous solution
References
List of references
- 1Janiel J. Reed (1989)The NBS Tables of Chemical Thermodynamic Properties: Selected Values for Inorganic and C1 and C2 Organic Substances in SI UnitsNational Institute of Standards and Technology (NIST)
- ^ ΔfH°, -1342.2 kJ · mol−1
- ^ ΔfG°, -1234.93 kJ · mol−1
- ^ S°, 176.61 J · K−1 · mol−1
- ^ Cp°, 142.13 J · K−1 · mol−1
- ^ ΔfH°, -1361.39 kJ · mol−1
- ^ ΔfG°, -1251.58 kJ · mol−1
- ^ S°, 168.2 J · K−1 · mol−1
- ^ ΔfH°, -2528.8 kJ · mol−1
- ^ ΔfH°, -4281.1 kJ · mol−1
- ^ ΔfH°, 609.358 kJ · mol−1
- ^ ΔfH°, -240.12 kJ · mol−1
- ^ ΔfG°, -261.905 kJ · mol−1
- ^ S°, 59.0 J · K−1 · mol−1
- ^ Cp°, 46.4 J · K−1 · mol−1
- ^ ΔfH°, -881.15 kJ · mol−1
- ^ ΔfG°, -727.75 kJ · mol−1
- ^ S°, 50.21 J · K−1 · mol−1